AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
To the AP Chemistry Student:
Welcome to my AP Chemistry class! I am looking forward to helping you gain a deeper appreciation for the
science of chemistry and how it impacts our lives. I hope you are looking forward to an exciting and
challenging year. Since you have elected to take this course, I assume you have the intelligence and motivation
needed to be successful. Your hard work will pay off, and you will find AP Chemistry to be a very rewarding
experience.
The Advance Placement Chemistry experience is designed to provide a full year of college-level chemistry, so
it places heavy demands on the student, especially in terms of the time commitment required. In fact, the
College Board suggests that students devote a minimum of five hours per week for individual study outside of
the classroom. The ultimate objective, of course, is to prepare you to take the AP Chemistry test in May 2015,
and in order to accomplish this, topics are covered very quickly. For this reason, most students take AP
Chemistry after they already completed a year of high school chemistry, since that provides them with a solid
foundation. In order to ensure the best start for you next fall, I prepared a Summer Assignment that reviews
many basic chemistry concepts.
It is important that everyone come to the first day of class well prepared! Extensive remediation is not an
option as we work towards our goal of becoming completely prepared for the AP Exam in early May, so seek
help early if you are experiencing difficulties.
Finally, I recommend that you spread out the Summer Assignment, rather than trying to complete it in the final
week of the summer! It takes time for a student to process, practice and subsequently learn chemistry at the
level necessary for success in AP Chemistry. Remember, AP Chemistry is an equivalent course to an
Introductory Chemistry college course, a full year program. Taking a college level course in high school is
difficult, and it requires commitment, hard work and time, but completion of a class like this is a great
investment in your education. Prepare yourself and arrive ready to learn!
You may want to use the following resources as help for the assignment that follows as well as throughout the
year. You may also find some of your own.
http://www.collegeboard.com/ap/students/chemistry/index.html
www.chemmybear.com
The following assignment will be reviewed in class beginning on the first day of school. I will take questions
on any problems you may have had from this assignment on the first few days of class. Therefore you need to
have your material with you on the first day. Please come prepared.
If you have any questions please feel free to call me at 678-201-6813 (if I do not answer, please leave your
name and a brief message and I will return your call) or email me at dsteiner@henry.k12.ga.us.
1. Review writing net ionic equations. You are expected to know the Solubility Rules on the attached page.
Memorize them!! We will have a quiz on Friday the first week of school over these.
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
2. Memorize all polyatomic ion formulas and charges. They are listed on the handout attached to this page.
Review these from Chem. I, as well. There are flash cards attached with some of them for you. Use them!
You will have a test over these on the third day of class. You also need to know the monatomic ions on the
attached page as well as be familiar with the important chemicals attached.
3. Complete the following assignment and bring to class with you on the first day of class.
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
AP Chemistry Summer Assignment
The following assignment is to be completed and brought on the first day of class.
DIRECTIONS: Solve the problems below, showing your setup, calculations, units and correct
Significant Figures (SigFigs). Neatly-written solutions are acceptable. (Points are deducted from AP
tests if correct SigFig rules and labels are ignored, so get into the habit of using them all of the time!)
1. Demonstrate that you know the correct use of significant figures (SigFig digits) by completing the following:
a. 738.90 m has _____ SigFgs.
b. 0.0304 g has _____ SigFigs.
c. 1.4 X 104 joules has _____SigFigs.
d. 1 dozen donuts has _____ SigFigs.
c. 40 mL has _____ SigFigs.
f. 800. m has _____ SigFigs.
2. A cylinder rod formed from silicon is 21.3 cm long and has a mass of 5.00 kg. The density of silicon is 2.33
g/cm3. What is the diameter of the cylinder? (The volume of cylinder is given by V = πr2h, where r is the radius
and h is the length.)
3. Calculate the following to the correct number of significant figures.
a. 1.27 g / 5.296 cm3 = ________________________
b. 12.235 g / 1.01 L = __________________________
c. 12.2 g + 0.38 g = _________________________
d. 17.3 g + 2.785 g = _______________________
e. 2.1m x 3.215m = _____________________
f. 200.1mi x 120 min = __________________
g. (17.6 + 2.838 + 2.3 + 110.77)g = _________________
4. A solid white substance A is heated strongly in the absence of air. It decomposes to form a new white
substance, B, and a gas, C. The gas has exactly the same properties as the product obtained when carbon is
burned in an excess of oxygen. Based on these observations, can we determine whether solids A and B and
the gas C are elements or compounds? Explain your conclusions for each substance.
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
Nomenclature
Name these binary compounds of two nonmetals.
4. N2O4
1. IF7
2. N2O5
5. As4O10
3. XeF2
6. SF6
7. PCl3
8. S2Cl2
Name these binary compounds with a fixed charge metal.
9. AlCl3
12. KI
10. MgO
13. SrBr2
11. BaI2
14. Na2S
15. CaF2
16. Al2O3
Name these binary compounds of cations with variable charge.
17. CuCl2
20. PbCl4
18. Fe2O3
21. Cu2S
19. SnO
22. HgS
23. AuI3
24. CoP
Name these compounds with polyatomic ions.
25. Fe(NO3)3
28. Ca(ClO3)2
26. NaOH
29. KNO2
27. Cu2SO4
30. NaHCO3
31. NH4NO2
32. Cu2Cr2O7
Name these binary acids
33. HCl
34. HI
Name these acids with polyatomic ions.
35. HClO4
36. H2SO4
37. HC2H3O2
38. H3PO4
39. HNO2
40. H2CrO4
41. H2C2O4
42. H2CO3
Name these compounds appropriately.
43. CO
44. NH4CN
45. HIO3
46. NI3
47. AlP
48. OF2
49. LiMnO4
50. HClO
51. HF
52. SO2
53. CuCr2O7
54. K2O
55. FeF3
56. KC2H3O2
57. MnS
Write the formulas.
58. Tin (IV) phosphide
59. Copper (II) cyanide
60. Magnesium hydroxide
61. Sodium peroxide
62. Sulfurous acid
63. Lithium silicate
64. Potassium nitride
65. Chromium (III)
carbonate
66. Gallium arsenide
67. Cobalt (II) chromate
68. Zinc fluoride
69. Dichromic acid
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
Solubility rules
Review solubility rules and identify each of the following compounds as soluble or insoluble in water.
70. Na2CO3
76. AgI
82. Li2O
71. CoCO3
77. Ni(NO3)2
83. Mn(C2H3O2)2
72. Pb(NO3)2
78. KI
84. Cr(OH)3
73. K2S
79. FeS
85. AgClO3
74. BaSO4
80. PbCl2
86. Sn(SO3)4
75. (NH4)2S
81. CuSO4
87. FeF2
Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility
of the products. If yes, identify the precipitate.
91. cobalt (III) bromide and potassium sulfide
88. silver nitrate and potassium chloride
92. ammonium hydroxide and copper (II)
89. magnesium nitrate and sodium carbonate
acetate
90. strontium bromide and potassium sulfate
93. lithium chlorate and chromium (III) fluoride
Balancing Equations
Balance the following equations with the lowest whole number coefficients.
94. S8 + O2  SO3
95. C10H16 + Cl2 
C + HCl
96. Fe + O2 
Fe2O3
97. C7H6O2 + O2  CO2 + H2O
98. KClO3  KCl + O2
99. H3AsO4 
As2O5 + H2O
100.
V2O5 + HCl  VOCl3 + H2O
101.
Hg(OH)2 + H3PO4  Hg3(PO4)2+H2
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
Stoichiometry, Limiting Reactants, and Gas Laws
102. Given the equation below, what mass of water would be needed to react with 10.0g of sodium
oxide?
Na2O + H2O  2NaOH
103. What mass of sodium chloride is formed along with 45.0g of oxygen gas?
2NaClO3  2NaCl + 3O2
104. What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen?
4NH3 + 5O2  4NO + 6 H2O
105. If the reaction in #104 is done with 25.0g of each reactant, which would be the limiting ;reactant?
106. Na2S + 2AgNO3  Ag2S + 2NaNO3
a. If the above reaction is carried out with 50.0g of sodium sulfide and 35.0g of silver nitrate, which
is the limiting reactant?
b. What mass of the excess reactant remains?
c. What mass of silver sulfide would precipitate?
107. What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium
hydroxide with 50.0g of aluminum?
6NaOH + 2Al  2Na3AlO3 + 3H2
108. White gold is an alloy that typically contains 45.0% by mass gold and the remainder is platinum. If 154 g of
gold are available, how many grams of platinum are required to combine with the gold to form this alloy?
109. What is the empirical formula of a compound that contains 53.73% Fe and 46.27% of S ?
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
110. In an experiment, a student gently heated a hydrated copper compound to remove the water of hydration.
The following data was recorded:
1. Mass of crucible, cover, and contents before heating = 23.4 g.
2. Mass of empty crucible and cover = 18.82 g.
3. Mass of crucible, cover, and contents after heating to constant mass = 20.94 g.
Calculate the percent by mass of water in the copper compound.
111. A hydrated compound has an analysis of 18.29% Ca, 32.37% Cl, and 49.34% water. What is its formula?
112. In Nature, strontium consists of four isotopes with masses and percent abundance of 83.9134 amu (0.50%),
85.9094 amu (9.9%) , 86.9089 amu (7.0 %) , and 87.9056 amu (82.6 %). Calculate the atomic mass of Sr.
113. Arsenic reacts with chlorine to form a chloride. If 1.587 g of arsenic reacts with 3.755 g of chlorine, what is
the empirical formula of the chloride?
114. Vanillin, a flavoring agent, is made up of carbon, hydrogen, and oxygen atoms. When a sample of vanillin
weighing 2.500g burns in pure oxygen, 5.79 g of carbon dioxide and 1.18 g of water are obtained. Calculate the
empirical formula of vanillin?
115. What is the molecular formula of each of the following compounds?
a. Empirical formula CH2 , molar mass =84g/mol
b. Empirical formula NH2Cl, molar mass = 51.5 g/mol
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
116.. Determine the empirical and molecular formula of each of Ibufuren, a headache remedy contains 75.6 %
C, 8.80 % H , and 15.5 % O by mass and a molar mass about 206 g/mol.
117. An open flask contains 0.200 mol of air. Atmospheric pressure is 745 mmHg and room temperature is
25˚C. How many moles are present in the flask when the pressure is 1.10 atm and the temperature is 33˚C?
118. On a warm day, an amusement park balloon is filled with 47.8 g He. The temperature is 33˚C and the
pressure in the balloon is 2.25 atm. Calculate the volume of the balloon.
119. Calculate the density of carbon dioxide gas at 27˚C and 763 torr.
120. Calculate the molarity of a solution that contains 20.0grams of sodium hydroxide in 200. ml of solution.
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
1. Become familiar with the following Formulas and Names for the Common Acids
and Compounds:
Hydrochloric Acid – HCl
Sulfuric Acid – H2SO4
Phosphoric Acid – H3PO4
Acetic Acid – HC2H3O2
Carbonic Acid – H2CO3
Nitric Acid – HNO3
AlK(SO4)2·12H2O alum
CH4 methane
C6H6 benzene
C10H8 naphthalene (mothballs)
CHCl3 chloroform
CH3OH methyl alcohol or methanol
(wood alcohol)
m. C2H5OH ethyl alcohol or ethanol
(drinking alcohol)
n. CH3COCH3 acetone
o. C3H5(OH)3 glycerin
p. C6H8O6 L-ascorbic acid (vitamin C)
q. CaCO3 chalk, marble, limestone
r. CaO quicklime
s. Ca(OH)2 slaked lime (lime water)
t. CaSO4 gypsum, plaster of paris
u. Fe3O4 or Fe2O3 rust
v. HCHO formaldehyde
w. H2O water
x. Hg quicksilver
y. K2CO3 potash
z. MgO magnesia
aa. MgSO4 epsom salts
bb. NH3 ammonia
cc. N2O laughing gas
dd. Na2CO3 soda ash
ee. NaCl table salt
ff. NaHCO3 baking soda
gg. NaNO3 saltpeter
hh. NaOCl bleach
ii. NaOH caustic soda or lye
jj. SiO2 sand, quartz
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
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AP Chemistry Summer Assignment 2014-2015
Ms. Steiner
Woodland High School
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